Chapter 13, Problem 124E

Interpretation Introduction

Interpretation: The general formula of an unknown salt is given to be $\text{BHCl}$ where $\text{B}$ a weak base is. The $\text{pH}$ value of a $0.10\text{M}$ solution of the unknown salt is $5.82$. The actual formula of the salt is to be stated.

Concept introduction: The $\text{pH}$ of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution.

The $\text{pH}$ of a solution is calculated by the formula, $\text{pH}=-\log \left[{\text{H}}^{+}\right]$

The sum, $\text{pH}+\text{pOH}=14$

The equilibrium constant for water is denoted by $K_{\text{w}}$ and is expressed as,

$K_{\text{w}}=\left[{\text{H}}^{+}\right]\left[{\text{OH}}^{-}\right]$

The value of $K_{\text{w}}$ is calculated by the formula,

$K_{\text{w}}=K_{\text{a}}\cdot K_{\text{b}}$